Solution Investigation Question: What are some of the key characteristics of unk

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Solution Investigation Question: What are some of the key characteristics of unknown sample of an aqueous solution containing an ionic compound?

1. Given that the cation is from Group 1A, what is the identity of the group 1A metal ion in your solution?  

2. Given that the ionic compound contains either chloride or hydroxide, how can you determine which? (Two pieces of evidence are required and one must be related to solubility rules)

3. What is the concentration of your solution? (Your unknown sample is known to be about 1 M, but you need to determine the concentration to 3 significant figures using titration. You should plan ahead so that you know approximately what volume of your sample you will need in order to use approximately 25 mL of 0.100 M sulfuric acid for the titration).

Resources Solubility Rules for Salts (lonic Compounds) Soluble Compounds Insoluble Compounds o Compounds of Group 1 elements o Carbonates (CO2), chromates (Cror2), Ammonium (NH4.)compounds o Chlorides (Cl), bromides (Br), and iodides oxalates (COr), and phosphates (POr), except those of the Group 1 elements and (I), except those of Ag, Hg2 and Pb NH o Nitrates (NOs), nitrites (NO:), acetates o Sulfides (S), except those of the Group 1 (CH CO2), chlorates (CIOs), and perchlorates (C1O:) and 2 elements and NH4. Hydroxides (OH) and oxides (O2), except those of the Group 1 and 2 elements, and NH o o Sulfates (SOr2), except those of Sr, Ba Pb2 and Hg

Explanation / Answer

1)

In aqueous solution ionic compoind undergoes ionizatoin.

In aqueous solution, the number of ions is related to the number of moles of the species is reltated to concentration by molarity.

since concentration is known, nuumber of moles can be calculated from the equation

concentration* volume of solution

moles= mass/molecular weight

Molecular weight= mass/ moles

The identity of group 1A metal can then be identified

2.) you need to add one of the dropper bottle solutions given to see if a precipitate forms.

Since we know it's OH we need to drop in a solution which will have a double replacement reaction.

If the product is insoluble, its OH. If not, it's Cl. But obviously it's OH because we are titrating. In this case, you may use an acid, and see if you form a precipitate of a salt.

With this you may know if you have a OH (All hidroxides of group 1 are soluble). If it's not, then you probably have a Cl.

However, like I stated before, we can have a clue of an OH because in the next step you begin to titrate so, it's an OH.

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